Statement I: Methyl orange is used as indicator in Na 2 CO 3 titrating against HCI solution. Statement II: The pH range of methyl orange is 3.1 to 4.5.
Solubility of M OH 2 in 0.1 M NaOH is K sp of M OH 2 = 2 × 10 – 24 M 3
Which salt can furnish H* il its aqueous solution?
Statement I: Increasing order of acidity of hydrogen halides is HF < HCI < HBr < HI. Statement II: While comparing acids formed by the elements belonging to the same group of the periodic table, H-A bond strength is a more important factor in determining acidity of an acid than the polar nature of the bond. HI bond is weaker than other halides, so lesser bond dissociation energy and more acidic nature.
p H of mixture containing three moles of NH 4 OH and half mole of H 2 SO 4 is p K b of NH 4 OH = 4 . 8
The strongest Bronsted base in the following anion is:
Which among the following salt solutions is basic in nature?
The solubility product for a salt of the type AB is 4 × 10 – 8 . What is the molarity of its standard solution?
p H of 0 .005 M weak monobasic acid is K a = 2 x 10 – 4
Which one of the following mixture cannot act like a buffer :
Which of the following is correct for finding out the P H of a buffer?
Percentage of base ‘B’ that forms BH + in a 0.1M aqueous solution of B will be( K b of base, B = 1 . 6 × 10 – 8 )
Conjugate acid of HPO 4 2- is
Identify Bronsted – Lowry acids in the reaction given below ? The correct answer is
Which of the following is not a conjugate acid – base pair ?
Among the following, relatively strong base is
Among the following, relatively weak base is
Which of the following acts as Lewis acid ?
Which of the following can acts as a Lowry-Bronsted acid as well as base ?
Which of the following is a Brnosted acid but not a Bronsted base ?
The conjugate base of hydrazoic acid is
Among the following a) On dilution, the pH of an acid increases b) A solution with pH = 5 is 100 times more basic than a solution with pH = 3 c) A solution with pH = 8 is 1000 times more acidic than a solution with pH = 11 d) The pH of 10 -9 M KOH is slightly greater than 7
For a weak acid ( is very small)
If the ionic product of water is at 35 0 C, its value at 10 0 C is
Each 10 -3 M of following four acids are taken. Their pH values are given in brackets. Which of the following is relatively stronger acid ?
For the ionization of ortho phosphoric acid , K 1 , K 2 , K 3 are successive ionization constants of the acid. Correct relation is
The first, second and third dissociation constants of a polybasic acid are in the order
Which of the following statement is correct ?
The pH of an aqueous solution is zero. Then the nature of the solution is
Few drops HCl is added to acetic buffer. The pH is mainted constant by
Which of the following is wrong ?
The compound whose 0.1 M solution is basic
Which of the following is correct for buffer [Salt = S; acid = A] ?
The nature of aqueous solution of CuSO 4 is
When NaCl is added gradually to the saturated solution of AgCl then which of the follwong plot is correct ?
A solution of Cu(NO 3 ) 2 in water is acidic due to
Aqueous solution of KCl is neutral because
In which of the following solutions, the solubility of AgCl will be maximum ?
The ionic product of water is 10 –14 . The H + ion concentration in 0.01M NaOH solution is
The H + ion concentration of a solution is 4×10 –5 M. Then the OH – ion concentration of the same solution is
One litre of water contains 10 -7 moles of H + ions. Degree of ionisation of water (in percentage) is
A 0.2M solution of formic acid is 3.2% ionised. Its ionisation constant is
The ionic product of water at 60 0 C is 9.55 × 10 –14 mole 2 lit –2 . The dissociation constant of water at the same temperature is
Four grams of NaOH solid are dissolved in just enough water to make 1 litre of solution. What is the [H + ] of the solution?
The pH of a weak monobasic acid is 3. It is diluted by 100 times, its pH of resulting solution will be
The dissociation constant (K a ) and percent of degree of dissociation ( α ) of a weak monobasic acid solution of 0.1M with a pH = 5 are respectively.
What is the pH of a solution obtained by dissolving 0.0005 mole of the strong electrolyte, calcium hydroxide, Ca(OH) 2 to form 100 ml of a saturated solution (aqueous)? (K w = 1.0 × 10 –14 mole 2 litre –2 )
The pH of a solution is 3.602. Its H + ion concentration is
The pH of 10 –3 M mono acidic base, if it is 1% ionised is
The pH of HCl is 3. Then the pH of NaOH solution having same molar concentration is
The pH of a solution is 5.0. To a 10 ml of this solution, 990 ml of water is added. Then the pH of the resulting solution is
At some high temperature, K w of water is 10 –13 . Then the pH of the water at the same temperature is
When 100 ml of N/10 NaOH are added to 50 ml of N/5 HCl, the pH of the resulting solution is
At certain temperature the K w of D 2 O is 10 –16 M. Then the pD of pure D 2 O at that temperature is
The pH of HCl is 1. The amount of NaOH to be added to 100 ml of such a HCl solution to get pH of 7 is
The pH of a base solution is 12.699. The amount of crystalline oxalic acid required to react with 2 lit of this base solution is (assume oxalic acid dissoiates completely)
Equal volumes of 0.5M NaOH and 0.3M KOH are mixed. Then the pH and pOH of resulting solution are respectively.
50 ml of H 2 O is added to 50 ml of 1 × 10 -3 M barium hydroxide solution. What is the pH of the resulting solution?
The pH of a sample of H 2 SO 4 is 1.3979. The percentage of the solution is 73.5% (w/w), the density of the solution is
The pH of 0.005 M Ba(OH) 2 is
The pH of a buffer solution is 4.745. When 0.044 mole of Ba(OH) 2 is added to 1 lit. of the buffer, the pH changes to 4.756. Then the buffer capacity is
pH of a buffer solution decreases by 0.02 units when 0.12g of acetic acid is added to 250 ml of a buffer solution of acetic acid and potassium acetate at 27 0 C. The buffer capacity of the solution is ?
P Ka of acetic acid is 4.74. The concentration of CH 3 COONa is 0.01M. The pH of CH 3 COONa solution is
The pH of the neutralisation point of 0.1 N NaOH with 0.1 N HCl is
The pH of 0.1M solution of the following salts increases in the order
When CO 2 is bubbled in excess of water, the following equilibrium is established. CO 2 + 2 H 2 O ⇌ H 3 O + + HCO 3 – K c = 3.8×10 –7 , pH = 6. What would be the HCO 3 – CO 2 ?
Hydrolysis constant of salt derived from strong acid and weak base is 2 × 10 –5 . The dissociation constant of the weak base is
Which of the following is the correct solubility of Ni OH 2 in 0.10 M NaOH? K sp of Ni OH 2 is 2 . 0 × 10 – 15 .
A buffer has equal volumes of 0.2 M NH 4 OH and 0.02 M NH 4 Cl . The P K b of the base is 5.The P H of buffer is
What is the solubility of Zr 3 PO 4 4 in water at 298 K?
Which of the following is least likely to behave as Lewis base?
Statement I : The acid-base pair that differs only by one proton is called a conjugate acid-base pair. Statement II: If Bronsted acid is a strong acid then its conjugate base is a weak base and vice-versa.
Statement I: Certain water soluble organic compounds like phenolphthalein and bromothymol blue behave as weak acids and exhibit different colours in their acid (HIn) and conjugate base In – forms. Statement II :
9.8 grams of H 2 SO 4 is dissolved in hundred litre solution. At 298 K, p H of the solution is
At 298 K, equal volumes of 0.15M Sulphuric acid and 0.3M Potassium hydroxide are mixed. p H of resultant mixture is
Solubility product of Silver chloride is 10 – 10 M 2 . Solubility of Silver chloride is 14 . 35 × 10 – x g / litre . Value of ‘ x ‘ is
p H of 0.1M Ammonium acetate solution at 298 K is 7.02. At 298 K, p H of ‘X’ M Ammonium acetate solution is 7.02. Value of X is
The hydrogen ion concentration of the oceans is about 2 × 10 – 9 M What is the pH?
Which is the strongest acid (pK a , value is given) ?
The solution of a sparingly soluble salt A x B y in water is ‘S” moles per. the solubility product has the value;
Following solutions were prepared by mixing different volumes of NaOH and HCl of different concentrations: A ) 60 mL M 10 HCl + 40 mL M 10 NaOH B ) 55 mL M 10 HCl + 45 mL M 10 NaOH C ) 75 mL M 5 HCl + 25 mL M 5 NaOH D ) 100 mL M 10 HCl + 100 mL M 10 NaOH pH of which one of them will be equal to 1?
The solubility of BaSO 4 in water is 2 . 42 × 10 – 3 g L – 1 at 298 K. The value of its solubility product K sp will be (Given molar mass of BaSO 4 = 233 g mol – 1 )
Which of the following salts will give highest pH in water?
Using the Gibb’s energy change, ∆ G ° = + 63 . 3 k J , for the following reaction, Ag 2 CO 3 ( s ) ⇌ 2 Ag ( a q ) + + CO 3 ( a q ) 2 – the K s p of Ag 2 CO 3 ( s ) in water at 25°C is R = 8 . 314 J K – 1 mol – 1
MY and NY 3 , two nearly insoluble salts, have the same K sp values of 6 . 2 × 10 – 13 at room temperature. Which statement would be true in regard to MY and NY 3 ?
What is the pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed?
Which one of the following pairs of solution is not an acidic buffer?
The dissociation constant of a weak acid is 1 × 10 – 4 . In order to prepare a buffer solution with a pH=5, the [Salt]/[Acid] ratio should be
p H of 0.005M Barium hydroxide solution at 298 K will be
Hydrolysis of salt is reverse of neutralization. Wrong match regarding salt hydrolysis among the following is
Which of the following fluoro compounds is most likely to behave as a Lewis base?
Strongest base among the following is
At 298 K, P H of 4% ionized 0.01M NH 4 OH solution will be
Solubility product is a measure of solubility of a sparingly soluble salt. Solubility product of Cr OH 3 is (S = Molar solubility)
P H of 0.1 M CH 3 COOH is K a = 10 − 5
Solubility of a salt is 0.09 M. It is classified as
Concentration of the Ag + ions in a saturated solution of Ag 2 C 2 O 4 is 2 . 2 x 10 – 4 mol L – 1 . Solubility product of Ag 2 C 2 O 4 is
Equal volumes of 0 . 02 M CH 3 COONa and 0 .2 M CH 3 COOH are mixed. Calculate H 3 O + of the mixture if p k a of acetic acid is 5
BF 3 , PF 3 , CF 4 , SiF 4 , PF 5 . How many can neither act like a Lewis acid nor like a Lewis base
Degree of ionization of CH 3 COOH is 0.1. Dissociation constant of its 0.01M solution at the same temperature will be
p H of 0.01M NaOH solution is ‘X’ & 0.05M H 2 SO 4 is ‘Y’. Value of (X–Y) is equal to
Solubility of AgCl is 1 .435 × 10 − 3 g / litre at 298 K. Solubility product of AgCl will be (GFW of AgCl = 143.5g)
Conjugate acid a of water is and conjugate base of ammonia is
p H of a mixture containing 100 ml of 0.1 M HCl and 200 ml of 0.05 M NaOH at 298K
Regarding aqueous solution of Sodium Cyanide, correct statements are A) Solution is alkaline in nature B) It undergoes anionic hydrolysis C) It turns pink by the addition of Phenolpthalein D) Its hydrolysis constant depends on K a of weak acid
At certain temperature, p H of 0.001 N solution of NaOH is 9. Ionic product of water at that temperature will be
Conjugate base of HSO 4 – is
Which of the following is relatively stronger acid ?
Al 3+ is a Lewis acid, because
Which of the following species acts as Bronsted base but not as acid ?
With increase in temperature, ionic product of water
At 298 K, on addition of NaOH to water
P H of a solution depends upon
Weakest base among the following is
Among the following a) pH of water decreases with increases in temperature b) pH of water decreases by the addition of base c) pH of water increases by the addition of acid d) At any temperature pH of water is equal to p K w 2
A buffer solution contains a weak acid HA and A – . When small quantity of NaOH is added to keep pH as constant, which of the following reaction takes place?
A physician wishes to prepare a buffer solution at pH = 3. 58 that efficiently resists a change in pH yet contains only small conc. of the buffering agents. Which one of the following weak acid together with its sodium salt would be best to use?
A basic buffer solution contains a weak base B and its conjugate acid BH + . On adding some HCl, which of the following reactions takes place to maintain constant pH ?
For the buffer solution containing NH 4 OH and NH 4 Cl, P H of the buffer solution can be increased by
Aqueous solution of which of the following shows lower pH ?
The pH of an aqueous solution of a salt is 10. The salt is
Aqueous solution of copper sulphate
Which of the following shows relatively higher pH ?
Which of the following salts undergoes anionic hydrolysis ?
Three sparingly soluble salts M 2 X, MX and MX 3 , have same value of solubility product. Their solubillities follow the order
Out of Ca 2+ , Al 3+ , Bi 3+ , Mg 2+ , Fe 3+ and Zn 2+ the reagents NH 4 Cl and aqueous NH 3 will precipitate
The solubility of BaSO 4 in water is . Its solubility product will be (molecular weight of BaSO 4 is 233)
Which of the following has the lowest value of K sp at 25 0 C ?
The solubility product of Hg 2 I 2 is equal to
Ionisation of NH 4 OH is supressed by the addition of NH 4 Cl, because
A buffer solution is used in
The [OH – ] of 0.005 M H 2 SO 4 is
At certain temperature, the H + ion concentration of water is 4 × 10 –7 M then the value of K w at the same temperature is
At 25 0 C, the hydroxyl ion concentration of a basic solution is 6.75 × 10 –3 M .Then the value of K w at same temperature is
The pH of 0.001 M acetic acd is
The dissociation constant of a weak acid is 10 -6 . Then the pH of 0.01 N of that acid is
The pH of 1.2% (w/v) aqueous solution of CH 3 COOH at 25 0 C is (pK a = 4.7)
The [OH – ] of a solution is 10 –10 . Its pH is
20cc of ‘x’ M HCl is exactly neutralised by 40cc of 0.05M NaOH. The pH of HCl solution is
The number of OH – ions in 1mL of solution having p H = 4 is
One litre of aqueous solution of H 2 SO 4 contains 4.9 g of the acid. 100 ml of this solution is taken in a 1 litre flask and diluted with water upto the mark. The P H of the dilute solution is
At 100 0 C, the pH of pure water is
The pH of a dibasic acid is 3.699. Its molarity is
The pH of HCl is 5. It is diluted by 1000 times. Its pH will be
Which one of the following statement is correct ?
20 ml of 0.4 M H 2 SO 4 and 80 ml of 0.2 M NaOH are mixed. Then the pH of the resulting solution is
The pH of a sample of KOH solution is 12.3979. The weight of solid KOH of 70% pure required to prepare 2.5 lit of this solution is
Solution of 0.1 N NH 4 OH and 0.1 N NH 4 Cl has pH 9.25. Then p K b of NH 4 OH is
When 0.1 mole of an acid is added to 2 lit of a buffer solution, the pH of the buffer decreases by 0.5. The buffer capacity of the solution is
When 11.2 g of KOH is added to one litre of ‘X’ M H 2 SO 4 solution, the pOH of the solution becomes 13.301. Then the value of ‘X’ is (assume no change in the volume of solution by the addition of KOH)
Which mixture forms a buffer when dissolved in 1 L of water?
4 mole of NH 4 OH and 1 mole of H 2 SO 4 are mixed and diluted to 1 lit solution. The pK b of NH 4 OH is 4.8 . The pH of solution is
Ka for HCN is 5 × 10 –10 at 25 0 C. For maintaining a constant pH of 9, the volume of 5M KCN solution required to be added to 10 ml of 2M HCN solution is
A solution contains equimolar concentration of a weak acid HA and its conjugate base A – . pKb of A – is 9. The pH of the solution is
A solution is prepared by mixing 100 ml of 0.1M NH 4 OH and 200 ml of 0.2M NH 4 Cl. pKb of NH 4 OH is 4.8. Then the pH of the solution is
If the solubility product of MOH is 1×10 –10 mol 2 .dm –2 , then the pH of saturated aqueous MOH solution will be
K sp of CaSO 4 .5H 2 O is 9 × 10 –6 , find the volume for 1g of CaSO 4 (Molecular weight = 136)
The K sp of a salt, having the general formula MX 2 , in water is 4 × 10 –12 . The concentration of M 2+ ions in the aqueous solution of the salt is
The precipitate of CaF 2 (K sp = 1.7×10 –10 ) is obtained when equal volumes of the following are mixed ?
Which of the following is most soluble in water?
The solubility product to different sparingly soluble salts are 1) XY = 4 × 10 –20 2) X 2 Y = 3.2 × 10 –11 3) XY 3 = 2.7 × 10 –31 The increasing order of solubility is
The solubility of PO 4 –3 is ‘x’ m/l in Ca 3 (PO 4 ) 2 . Then its K sp is
If the K SP of a sparingly soluble salt, A 3 B 2 in water is 1.08 × 10 –8 mol 5 L –5 , its solubility in mol L –1 is
The molar solubility of sparingly soluble salt M x X y in its saturated solution at a given temperature is ‘S’. The correct relation between ‘S’ and K sp of it is (K sp = solubility product).
The molar solubility of M(OH) 3 in 0.4 M MX 3 solution in terms of solubility product of M(OH) 3 is
The solubility of PbSO 4 in 0.01M Na 2 SO 4 solution is (K sp of PbSO 4 is 1.25 × 10 –9 )
The molar solubility of PbI 2 in 0.2M Pb(NO 2 ) 2 solution in terms of solubility product, K sp
To 100ml of 0.1 M AgNO 3 solution, solid K 2 SO 4 is added. The concentration of K 2 SO 4 that shows the precipitation is (K sp for Ag 2 SO 4 = 6.4 × 10 –5 m 3 /l 3 )
Statement I : Aqueous solution of ammonium acetate is neutral. Statement II : Dissociation constants of NH 4 OH (K b ) and that of CH 3 COOH (K a ) are nearly equal.
Statement I : Aqueous solution of Na 2 CO 3 shows pH > 7. Statement II : Salt of strong base and weak acid undergoes anionic hydrolysis.
Statement I : The pH range of any indicator is from pK In – 1 to pK In + 1 Statement II : The pH of indicator is given as, pH = pK ln + log ln – [ Hln ] . Colour change of indicator takes place when ln – = [ Hln ]
Statement I : Al H 2 O 6 3 + is a stronger acid than Mg H 2 O 6 + 2 Statement II : Size of Al H 2 O 6 3 + smaller than Mg H 2 O 6 + 2 and posses more effective nuclear charge.
Statement I : In the acid – base titration involving strong base and weak acid, methyl red can be used as an indicator. Statement II : Methyl red does not changes its colour in the pH range 4.2 to 6.3.
Statement I : When 0.1M weak diprotic acid H 2 A dissociates with its dissociation constants K a1 = 10 -3 and K a2 =10 -8 and , then [A –2 ] is almost equal to 10 –3 M. Statement II : Since K a 2 < < K a 1 for 0.1 M H 2 A, so [A –2 ] is considerable w.r.t. [HA – ].
Statement I : Sparingly soluble salts AB and XY 2 with the same solubility product, will have different solubility. Statement II : solubility of sparingly soluble salt depend upon solubility product.
Statement I : Solubility of sparingly soluble salt decreases due to common ion effect. Statement II : Solubility product constant does not depend on common ion effect.
Statement I : 0.1M NaCN + 0.05M HCl solution on mixing in equal volume forms a buffer solution Statement II : The solution after mixing contains a weak acid and its conjugate base and thus acts as buffer
Statement I : A very dilute acidic solution of Cd 2+ and Ni 2+ gives yellow precipitate of CdS on passing hydrogen sulphide. Statement II : solubility product of CdS is more than that of NiS.
Three sparingly soluble salts M 2 X , MX and MX 3 have the same solubility product. Their solubilities will be in the order
The solubility of a sparingly soluble compound MX 2 at 25 0 C is 5 . 0 × 10 – 3 mol / L . Its solubility product at that temperature is
solubility product of salt MX 4 is K SP and solubility S mol/L are related as
The solubility of a sparingly soluble salt AB 2 in water is 1 . 0 × 10 – 5 mol L – 1 . Its solubility product is
The solubility product of a salt having general formula MX 2 in water is 4 × 10 – 12 . The concentration of M 2 + ions in the aqueous solution of the salt is
The solubility product K sp of the sparingly soluble salt MX at 25 0 C is 2 . 5 × 10 – 9 . The solubility of the salt (in mol L – 1 ) at this temperature is
pH of a buffer solution decreases by 0.02 units when 0.12 g of acetic acid is added to 250 mL of a buffer solution of acetic acid and potassium acetate at 27 o C . The buffer capacity of the solution is
The pH of a buffer is 6.745. When 0.01 moles of NaOH is added to 1 litre of it, the pH changes to 6.832. Its buffer capacity is
For preparing a buffer solution of pH 6 by mixing sodium acetate and acetic acid, the ratio of the concentration of salt and acid should be K a = 10 – 5
pH of a mixture containing 0.10 M X – and 0.20 M HX is pK b X – = 4
The total number of different kind of buffers obtained during the titration of H 3 PO 4 with NaOH are
Which may be added to one litre of water to act a buffer ?
If an acidic indicator HIn ionizes as HIn ⇌ H + + In – . To which maximum pH value its solution has distinct colour characteristic of HIn.
Statement 1 : Addition of HCl(aq) to HCOOH(aq) decreases the ionization of HCOOH(aq). Statement 2 : Due to common ion effect of H + , ionization of HCOOH decreased.
Statement 1 : Acids that have more than one proton that can be donated to base are called polyprotic acids. Statement 2 : For all diprotic acids, the equilibrium constant K a 2 , for the second stage of ionisation is smaller than the equilibrium constant, K a 1 , for the first stage of ionisation.
Statement 1 : 0.20 M solution of NaCN is more basic than 0.20 M solution of NaF. Statement 2 : K a of HCN is very much less than that of HF.
Statement 1 : pH of 10 – 7 M HCl is less than 7 at 25 o C . Statement 2 : At very low concentration of HCl, contribution of H + from water is considerable.
Which of the following molecules acts as a Lewis acid ?
What is the OH – in the final solution prepared by mixing 20.0 mL of 0.050 M HCl with 30.0 mL of 0.10 M Ba OH 2 ?
Statement 1 : A solution of FeCl 3 in water produces brown precipitate on standing. Statement 2 : Hydrolysis of FeCl 3 takes place in water.
Statement 1 : BaCO 3 is more soluble in HNO 3 than in plain water. Statement 2 : Carbonate is a weak base and reacts with the H + from the strong acid, causing the barium salt to dissociate.
Solubility of AgCl in water, 0.01 M CaCl 2 , 0.01 M NaCl and 0.05 M AgNO 3 are S 1 , S 2 , S 3 and S 4 respectively, then
Statement 1 : Solubility of AgCl in NH 3 aq is greater than in pure water. Statement 2 : When AgCl dissolve in NH 3 aq , complex ion Ag NH 3 2 + formation takes place and solubility equilibrium of AgCl shifted in forward direction.
What would be the pH of an ammonia solution if that of an acetic acid solution of equal strength is 3.2 ? Assume dissociation constants for NH 3 and acetic acid are equal.
In which case pH will not change on dilution
Which of the following is/are correct?
Select the correct statement (s) out of the following.
What is the P H of a buffer containing 0.09 M CH 3 COOH and 0.15 M of potassium acetate? K a = 1 . 8 × 10 – 5 , log 5 = 0 . 699 , log 3 = 0 . 4771 , log 1 . 8 = 0 . 2553
Statement-I: The ionisation of hydrogen sulphide in water is low in the presence of hydrochloric acid. Statement-II: Hydrogen sulphide is a weak acid
Statement 1: The aqueous solution of FeCl 3 is basic in nature. Statement 2: FeCl 3 hydrolyses in water.
p H of a mixture containing 100 ml of 0.1M acetic acid and 100 ml of 0.2M sodium acetate is 5.1. p K a of acetic acid is
To a one litre solution containing 4 grams of sodium hydroxide, 9.8 grams of sulphuric acid is added p H of the solution at 298 K is
If the solubility product of CuS in 6 x 10 -16 , calculate the maximum molarity of CuS in an aqueous solution.
According to Arrhenius theory, acids are substances that dissociate in water to give X ions and bases are substances that produce Y ions. X and Y respectively are
“An acid is a substance that is capable of donating a hydrogen ion H + and bases are substances capable of accepting a hydrogen ion, H + ” . The above statement is justified by
In the reaction, X and Y respectively are
The solubility product K sp of the sparingly soluble salt MX at 25°C is 2 . 5 × 10 – 9 . The solubility of the salt (in mol L – 1 ) at this temperature is
Three sparingly soluble salt that have same solubility products are given below I. A 2 X II. AX III. AX 3 Their solubilities order in a saturated solution will be
If S 1 , S 2 , S 3 and S 4 are the solubilities of AgCl in water, in 0.01 M CaCl 2 , in 0.01 M NaCl and in 0.05 M AgNO 3 respectively at a certain temperature, the correct order of solubilities is
Match the Column I with Column II and choose the correct option from the codes given below. Column I (Hydrolysis of the salts) Column II (Example) A. Weak acid and strong base 1. NH 4 Cl B. Strong acid and weak base 2. CH 3 COONH 4 C. Weak acid and weak base 3. CH 3 COONa Codes
Match the column I (molecules/ions) with column II (acid/base) and choose the correct option from the codes given below. Column I Column II A. Mg 2 + 1. Hard acid B. H 2 O 2. Soft acid C. R 3 P 3. Hard base D. Ag + 4. Soft base Codes
Pb ( s ) + Hg 2 SO 4 ( s ) ⇌ PbSO 4 ( s ) + 2 Hg ( 1 ) E cell o = 0 .92 V K sp ( PbSO 4 ) = 2 × 10 − 8 , K sp ( Hg 2 SO 4 ) = 1 × 10 − 6 Hence, E cell for a cell containing saturated solutions of the two salts in their respective electrodes would be: Given [antilog (0.141) = 1.38]
Four grams of NaOH is dissolved in ten litre solution. At 298 K, p H of the solution is
0.1 moles of H 2 SO 4 is dissolved in hundred litre solution. At 298 K, p H of the solution is
At 298 K, equal volumes of 0.15M Sulphuric acid and 0.3M Potassium hydroxide are mixed. p H of resultant mixture is
p H of 0.1M Ammonium acetate solution at 298 K is 7.02. At 298 K, p H of ‘X’ M Ammonium acetate solution is 7.02. Value of X is
The hydroxide ion concentration of a wine is 8 x 10 -11 M . What is the pH of the wine?
Which will make basic buffer?
pH of a saturated solution of Ca ( OH ) 2 is 9 . The solubility product K sp of Ca ( OH ) 2 is
Conjugate base for Bronsted acids H 2 O and HF are
Which of these is least likely to act as a Lewis base?
Accumulation of lactic acid HC 3 H 5 O 3 , a monobasic acid in tissues leads to pain and a feeling of fatigue. In a 0.10 M aqueous solution, lactic acid is 3.7% dissociates. The value of dissociation constant, K a , for this acid will be
The values of K sp of CaCO 3 and CaC 2 O 4 are 4 . 7 × 10 – 9 and 1 . 3 × 10 – 9 respectively at 25 o C . If the mixture of these two is washed with water, what is the concentration of Ca 2 + ions in water?
The percentage of pyridine C 5 H 5 N that forms pyridinium ion C 5 H 5 N + H in a 0 . 10 M aqueous pyridine solution K b for C 5 H 5 N = 1 . 7 × 10 – 9 is
From the following sparingly soluble salts, identify the salt with maximum solubility
Solubility product is a measure of solubility of a substance. Solubility product of a sparingly salt, AB 2 is 32 × 10 − 18 . B – in the saturated solution is
The solubility of AgCl ( s ) with solubility product 1 . 6 × 10 – 10 in 0 . 1 M of NaCl solution would be
H 3 O + of acidic buffer is 10 – 5 and ionization constant of the weak acid is 10 − 6 . Then [acid] : [salt] is
Which one of the following is a Lewis base
CH 3 COOH + H 2 O ⇌ CH 3 COO – + H 3 O + . In this reaction, H 2 O acts like
Equal volumes of 0.2 M HCl and 0.4 M H 2 SO 4 are mixed. p H of the resultant mixture is
Consider the following mixtures. The mixture in which Common ion effect is not observed is
Find out the solubility of Ni ( OH ) 2 in 0 . 1 M NaOH . Given that the ionic product of Ni ( OH ) 2 is 2 x 10 – 15
The pH of 0.01 M NaOH (aq) solution will be
Which of the following cannot act both as Bronsted acid and as Bronsted base?
The molar solubility of CaF 2 K sp = 5 .3 × 10 − 11 in 0.1 M solution of NaF will be
p H of 0.1M weak monobasic acid is 4. Ionisation constant of weak acid is
Consider the following mixtures. Which one of the following mixture has a p H = 2
I(salt) II Type of Hydrolysis A) CuSO 4 I) Cationic and anionic hydrolysis B) KNO 3 II) Anionic hydrolysis C) NaCN III) Cationic hydrolysis D) HCOONH 4 IV) No hydrolysis Correct match is
p H of a saturated solution of M ( OH ) 2 is 10. Solubility product of M ( OH ) 2 will be
Solubility product of M OH 3 is 3 × 10 − 18 . Molar solubility of M OH 3 in 0.01M KOH will be
Statement I : Mixture of 50 ml of 0.2M NH 4 OH and 25ml of 0.1M HCl is a basic buffer Statement II : Hydrolysis of a salt is reverse of neutralization
Which one of the following has only a conjugate acid but no conjugate base :
Conjugate base of hydrogen atom is
Buffer capacity of an acid buffer is maximum when
Solubility product of a sparingly soluble salt P 2 Q is 4 × 10 − 15 M 3 . P + in its saturated solution is
Solubility of sparingly soluble salts is influenced by various factors.Solubility of AgCl is minimum in
p H of 10 ml of weak monoprotic acid is 4. To increase p H of this solution by one unit the volume of water that must be added is
Equimolar solutions of the following substances were prepared separately. Which one of these, record the highest p H value.
Acetic acid dissociates as CH 3 COOH CH 3 COO – + H + . If a little amount of sodium acetate is added to its aqueous solution
At equilibrium, the addition of CN – ions would
Which of the following is a Lewis acid ?
Which of the following is a Lewis acid ?
O 2 2- is the conjugate base of
The equilibrium constant for this reaction is approximately 10 -3 HPO 4 ( aq ) 2 – + HCO 3 ( aq ) – ⇌ H 2 PO 4 ( aq ) – + CO 3 2 – ( aq ) Which is the strongest conjugate base in this reaction?
Incorrect statement in the following is
Of the given anions, the strongest Bronsted base is
The unit of ionic product of water is
Which of the following is neither Bronsted acid nor Bronsted base ?
According to Lewis ‘CO’ is
Ionic product of water depends on
At 298 K, the [H 3 O + ] of a solution is 2 x 10 -9 M. The nature of the solution is
At 100 0 C, the value of is
At 25 0 C , for an acid
For a strong acid,
The pH of 40 ml of a 0.02 M HCl will not be changed by adding
At any temperature, the proton concentration of water is
For a conjugate acid-base pair, K a and K b are related as
Which of the following is relatively stronger base ? (pK b values are given in brackets)
Weakest conjugate base is obtained from
A,B,C are three solutions prepared by adding a salt, and acid and a base respectively. Then ionic product of water will
Strongest acid among the following is
Which of the following is not correct ?
Which of the following acts as a Lewis acid in the following reaction SnCl 4 + 2 Cl – SnCl 6 – 2 ?
Which of the following statement is not correct ?
The dissociation constants of four monobasic acids HA, HX, HY and HD are respectively 6 x 10 -4 , 5 x 10 -5 , 3.6 x 10 -6 and 7 x 10 -10 . The pH values of their 0.1M solutions is
Which of the following is relatively stronger acid ? (K a values are given in brackets)
Which of the following is correct?
The dissociation constant of H 2 S and HS – are respectively 10 -7 and 10 -13 . The pH of 0.1M aqueous solution of H 2 S will be
The dissociation constants of monobasic acids A, B, C and D are respectively. The pH values of their 0.1 molar aqueous solutions are in the order
At any temperature, pH + pOH is equal to
Which of the following is wrong ?
If the dissociation constants of two weak acids A & B are K 1 & K 2 , then the relative strengths of A & B are given by
The successive dissociation constants Ka 1 , Ka 2 and Ka 3 of ortho phosphorous acid (H 3 PO 3 ) are
Which of the following is a weak electrolyte ?
At infinite dilution, the percentage ionisation of both strong and weak electrolytes is
For acetic acid and sodium acetate buffer, addition of which of the following increases the pH ?
For a weak acid, the concentration of H + ions is given by
From the following table Buffer solution volume of 0.1M weak acid(in ml) volume of 0.1M sodium salt of weak acid (in ml) I. 4.0 4.0 II. 4.0 40.0 III. 40.0 4.0 IV. 0.1 10 Which of the two sets of buffer solutions have least pH ?
The correct expression for OStwald’s dilution law for a solution of weak electrolyte is (if initial number of moles = 1)
Which of the following pair of solutions does not form a buffer solution ?
Which of the following mixture acts as buffer solution ?
A solution that has reserve acidity (or) alkalinity is called
Buffer capacity of an acidic buffer solution is maximum when a) pH = pK a (b) [salt] = [acid] c) pK a = 7 d) [H + ] = pK a
An acidic buffer contains
To a buffer solution of CH 3 COOH and CH 3 COONa, some HCl is added. Then the reaction involved is
The pH of 0.1 M solution of the following compounds increases in the order
Nature of 0.1 M solution of sodium sulphite is
A salt of weak acid and weak base undergoes
Aqueous solution of salt of strong acid and weak base
The hydrolysis constant of MX is ( Given K b of MOH is 2 × 10 – 6 and K a of HX is 5 × 10 – 7 )
Statement I : Aqueous solution of NaHCO 3 is acidic in nature Statement II : NaHCO 3 is acid salt.
The hydrolysis constant of CH 3 COONa is given by
Aqeous solution of salt of weak acid and strong base
Which of the following salts, does not undergo hydrolysis ?
MX is the salt of weak base, MOH and weak acid, HX. Aqueous solution of MX is
The hydrolysis constant of ammonium acetate is given by
The solubility of calcium phosphate in water is x mol L – 1 at 25 0 C. Its solubility product is equal to
Which of the following salt is least soluble ?
At a certain temperature, the solubility of the salt M m A n in water is ‘s’ moles per litre. The solubility product of the salt is
If the solubility product of MOH is 1 × 10 – 10 mol 2 dm -6 then the pH of its aqueous solution will be
In qualitative analysis, to identify the II A group sulphides, HCl is added to salt solution before the addition of H 2 S. Because
For the electrolyte of type, A 2 B , K sp is given. Then its solubility is calculated by
Dissociation of acetic acid is suppressed in presence of
Why only As +3 gets precipitated as As 2 S 3 and not Zn 2+ as ZnS when H 2 S is passed through an acidic solution containing As +3 and Zn +2 ?
The addition of NaCl to AgCl decreases the solubility of AgCl, because
The correct representation for solubility product of SnS 2 is
In the following reaction, . As KI is added, the equilibrium is shifted towards right giving more AgI precipitate, because
Which of the following is precipitated as sulphide in acidic solutions
The molar solubility in mol.lit -1 of a sparingly soluble salt MX 4 is S. The corresponding solubility product K sp is given by the relation.
Among the following statements a) If two salts have equal solubility then their solubility products are equal. b) BaSO 4 is more soluble in water than in dil.H 2 SO 4 c) When KI is added to PbI 2 , the [Pb 2+ ] decreases d) In any solution containing AgCl, the value of [Ag + ,Cl – ] is constant at constant temperature.
Three sparingly soluble salts that have same solubility products are given below : I) A 2 X II) AX III) AX 3 Their solubilities in a saturated solution will be such that
To Ag 2 CrO 4 solution over its own precipitate , ions are added.This result in
Let the solubility of an aqueous solution of Mg(OH) 2 be ‘x’; then its K sp is
If the solubility of Lithium sodium hexafluoro aluminate Li 3 Na 3 (AlF 6 ) 2 is ‘a’ mole/litre, its solubility product is equal to
Solubility of BaF 2 in a solution of Ba(NO 3 ) 2 will be represented by the concentration term
2 mole each of CH 3 OH & CH 3 COOH are taken and heated in the presence of conH 2 SO 4 so that equilibrium is established. If K C for esterfication process is 4, mass of ester present at equilibrium (in gm) is
The number of H 3 O + ions present in 10 ml of water at 25 0 C is
The dissociation constant of water at 10 0 C is 5.31 × 10 –17 . The ionic product of water is
At 100 0 C, ionic product of water is 51.3 ×10 –14 M 2 . Then dissociation constant of water at 100 0 C is
The hydrogen ion concentration of 0.2M CH 3 COOH which is 4% ionised is
Degree of dissociation of 0.1 N CH 3 COOH is (K a = 1.0 × 10 –5 )
The pH of a weak mono basic acid is 5. The degree of ionisation of acid in 0.1 M solution is
The pH of 10 –8 M aqueous HCl is
Equal volumes of two solutions with pH =3 and pH = 11 are mixed. Then the pH of resulting solution at 298 K is
The pH of a solution is 4.301. To 50 ml of this solution 200 ml of water is added. Then the pH of resulting solution is
The pH of a solution is 12. Number of H + ions present in 1 ml of this solution at 25 0 C is
The pH of a solution is 3.0. This solution is diluted by 100 times. Then the pH of the resulting solution is
Equal volumes of 0.1 M potassium hydroxide and 0.1 M sulphuric acid are mixed. The pH of resulting solution is
The pH of a solution is 6. Its [H 3 O + ] is decreased by 1000 times. Its pH will be
The pH of solution is 9. It is times more basic than a solution with pH = 6.
The pH of a 1 lit solution is 2. It is diluted with water till its pH becomes 4. How many litres of water are added ?
The pH of a solution is 11. It is diluted by 1000 times. Then the pH of resulting solution is
To change the pH of a solution from 1 to 1.301 which of the following should be adopted ?
The concentration of oxalic acid is ‘X’ mol lit -1 40 ml of this solution reacts with 16ml of 0.05 M acidified KMnO 4 . What is the pH of ‘X’ M oxalic acid solution ? (Assume that oxalic acid dissociates completely)
An acidic buffer contains 0.06 M salt and 0.02 M acid. The dissociation constant of acid is 10 -4 . The pH of the buffer solution is
Urine normally has a pH of 6.0. A patient eliminates 1.3 litres of urine per day. How many moles of H + ions does he eliminate in a day ?
50 ml of 0.1 M solution of sodium acetate and 50 ml of 0.01 M acetic acid are mixed. The pKa of acetic acid is 4.76. The pH of the buffer solution is
50 ml of 0.2N H 2 SO 4 is mixed with 100 ml of 0.4N KOH solution and 1.85 lit of distilled water is added. The pH of resulting solution is (log 1.5 = 0.176)
In an acidic buffer solution (pH = 4.4), the concentration ratio of acid and salt is 2 : 1. The value of dissociation constant of weak acid may be
An acidic buffer contains equal concentrations of acid and salt. The dissociation constant of acid is 10 -5 . The pH of the buffer solution is
Which of the following solution will have pH closer to 1.0 ?
Find the change in pH when 0.01 mole CH 3 COONa is added to one litre of 0.01M CH 3 COOH solution (pKa = 4.74 )
A one litre solution contains 0.08 mole of acetic acid (K a = 1.75 × 10 –5 ). To this solution, 0.02 mole of NaOH is added. Then the pH of resulting solution is [log 1.75 = 0.243]
A buffer solution consists of 1 mole each of HA and its conjugate base A – . Addition of which of the following decreases the pH of buffer?
2 g of NaOH per 250 ml of solution is added to a buffer solution of buffer capacity 0.2. Then the change in pH is
20 ml of 0.1 M acetic acid is mixed with 50ml of potassium acetate. K a of acetic acid = 1.8 × 10 –5 at 27 0 C. The concentration of potassium acetate if pH of the mixture is 4.8
If the pK a of CH 3 COOH and pK b of NH 4 OH are the same as 4.76, the pH of an aqueous solution of ammonium acetate is
A buffer solution is prepared by mixing CH 3 COONa and CH 3 COOH. The pK a of acetic acid is 4.74. To maintain the pH of the buffer solution as 6.04, the concentration ratio of CH 3 COONa and CH 3 COOH to be maintained is
The pH of an aqueous solution of CH 3 COONa of concentration C(molarity) is given by
The pH of aqueous solution of NH 4 CN (K a of HCN is 9.2 × 10 –10 & K b of NH 4 OH is 1.8 × 10 –5 )
The hydrolysis constant of NaX (K a of HX is 2 × 10 –6 ) is
Which of the following statements is true?
What is the minimum concentration of SO 4 2– required to precipitate BaSO 4 in a solution containing 1.0 × 10 –4 mole/lit of Ba 2+ ? (K sp of BaSO 4 = 4 × 10 –10 )
If the solubility of Ca(OH) 2 is 3 , What is its solubility product ?
The correct order of increasing [H 3 O + ] in the aqueous solution is
The solubility product of BaSO 4 at 18 0 C is 1.5 × 10 –9 . Its solubility (mole lit –1 ) at the same temperature is
At 25 0 C, in the saturated solution of Ag 2 CrO 4 . If concentration of CrO 4 –2 ion is 1 × 10 –4 mol/l, then the solubility product of Ag 2 CrO 4 at 25 0 C is
Calomel is mercurous chloride which exist as a dimer. If its molar solubility in water is 10 –2 M, then its solubility product will be
The solubility of CaF 2 is 2 × 10 –4 mole/litre. Its solubility product is
In a saturated aqueous solution of AgBr, conc. of Ag + ion is 1× 10 –6 mol/lit. If K sp for AgBr is 1×10 –12 , then concentration of Br – in the solution is
The solubility of AgCl in 0.1M NaCl is (K sp of AgCl = 1.2 × 10 –10 )
Let the solubilities of AgCl in H 2 O, 0.01M CaCl 2 , 0.01M NaCl and 0.05M AgNO 3 be S 1 , S 2 , S 3 and S 4 respectively. What is the correct relationship between these quantities ?
Statement I : On mixing 500mL of 10 –6 M Ca 2+ ion and 500 mL of 10 –6 MF -1 ion, the precipitate of CaF 2 will be obtained K sp (CaF 2 ) = 10 –18 Statement II : If K sp is more than ionic product, precipitate will be obtained.
Statement I : Benzoic acid (Ka = 6.5×10 –5 ) is stronger acid than acetic acid (Ka = 1.74×10 –5 ). Statement II : Larger the value of K a , greater is the acidity.
Statement I : Decreasing order of strength of bases is as CH 3 CH 2 – > NH 2 – > HC ≡ C – > OH – Statement II : Acidic stength order is C 2 H 6 < NH 3 < C 2 H 2 < H 2 O
Statement I : All strong monoprotic acid with same concentration in dilute solution show same pH. Statement II : Water shows leveling effect.
Statement I : Since HClO 4 is a stronger acid than H 2 SO 4 , HCl and HNO 3 ,and therefore it has a greater tendency to donate proton in comparison to others. Statement II : Perchloric acid is stronger acid than H 2 SO 4 in acetic acid.
Statement I : Methyl orange is not a suitable indicator if the acid is a weak acid like acetic acid. Statement II : Methyl orange is a weak base.
Statement I : NaCl + HCl does not experience common – ion effect. Statement II : Both NaCl and HCl are strong electrolytes.
Statement I : In presence of dilute HCl, Zn 2+ is not precipitated by S 2– ions. Statement II : The dissociation of H 2 S is suppressed by addition of dilute HCl.
If equal volumes of BaCl 2 and NaF solutions are mixed, which of these combinations will not give a precipitate? Substance = BaF 2 k sp = 1.7 × 10 -7
helps to maintain pH of blood between 7.26 to 7.42.
The third group radicals are precipitated as hydroxides by means of NH 4 OH in presence of NH 4 Cl because
Identify the wrong match from the following Set – I Set – II A) HCl – NaOH 1) Methyl orange B) HCl – NH 4 OH 2) Methyl red C) CH 3 COOH-NaOH 3) Any indicator D) CH 3 COOH-NH 4 OH 4) Phenolphthalein 5) No suitable indicator
The dissociation constants of H 2 S and HS –1 are respectively 10 –7 and 10 –13 . The P H of the aqueous solution containing 0.2 mole of H 2 S dissolved in 1 lit water is
If Ksp of Ag 2 CO 3 is 8×10 –12 , the molar solubility of Ag 2 CO 3 in 0.1M AgNO 3 is :
Solubility of AgCl at 20 0 C is 1.435 × 10 –3 g per litre. The solubility product of AgCl is
Calomel is mercurous chloride which exist as a dimer. If its molar solubility in water is 10 -2 M then its solubility product will be
The solubility of Ca(OH) 2 in water is 6 ×10 –6 M. The solubility of Ca(OH) 2 in a buffer solution of pH = 10 is
Statement I : NaHCO 3 is an acidic salt Statement II : Aqueous solution of NaHCO 3 is acidic
Which of the following is an example of weak electrolyte
A solution consists of 0.2 M NH 4 OH and 0.2 M NH 4 Cl. If K b of NH 4 OH is 1.8 × 10 –5 , the [OH – ] of the resulting solution is
When rain is accompanied by a thunderstorm, the collected rain water will have a pH
Hydrogen ion concentration in mol/L in a solution of pH = 5.4 will be
10 – 6 M NaOH is diluted by 100 times. The pH of diluted base is
The pK a of a weak acid, HA, is 4.80. The pK b of a weak base, BOH, is 4.78. The pH of an aqueous solution of the corresponding salt, BA, will be
An acid HA ionizes as HA ⇌ H + + A – The pH of 1 M solution is 5. Its dissociation constant would be
Which statement is not true ?
How many litres of water must be added to 1 L of an aqueous solution of HCl with a pH of 1 to create an aqueous solution with pH of 2 ?
If K h (hydrolysis constant) for anilinium ion is 2 . 4 × 10 – 5 M , then K b for aniline will be
The aqueous solution of potash alum is acidic due to hydrolysis of
Which is least soluble in water ?
A white salt is readily soluble in water and gives a colour less solution with a pH of about 9. The salt would be
The aqueous solution of FeCl 3 is acidic due to
pH for the solution of salt undergoing anionic hydrolysis (say CH 3 COONa ) is given by
If acetic acid is mixed with sodium acetate, then H + ion concentration will be
An aqueous solution of sodium carbonate has a pH greater than 7 because
Which of the following salts when dissolved in water will get hydrolysed ?
An aqueous solution of CH 3 COONa will be
In which of the following salt hydrolysis takes place
From separate solutions of sodium salts, NaW, NaX, NaY and NaZ have pH 7.0, 9.0 10.0 and 11.0 respectively. When each solution was 0.1 M, the strongest acid is
Which one of the following salt is most acidic in water ?
Which is the correct alternate for hydrolysis constant of NH 4 CN ?
When 0.1 mole of solid NaOH is added in 1 L of 0.1 M NH 3 ( aq ) then which statement is going to be wrong ? K b = 2 × 10 – 5 , log 2 = 0 . 3
Which of the following aqueous solution will have a pH less than 7.0 ?
Hydrolysis constant for a salt of weak acid and weak base would be
Which salt can be classified as an acid salt ?
Which salt will give basic solution on hydrolysis ?
HA is a weak acid and BOH is a weak base. For which of the following salts the extent of hydrolysis is independent of the concentration of the salt in its aqueous solution
0.5 M ammonium benzoate is hydrolysed to 0.25 percent, hence its hydrolysis constant is
The pH of 0.02 M NH 4 Cl ( aq . ) pK b = 4 . 73 is equal to
pH of water is 7. When a substance Y is dissolved in water, the pH becomes 13. The substance Y is a salt of
Which of the following will not be hydrolysed ?
100 ml of 0.1 M CH 3 COOH are mixed with 100 ml of 0.1 M NaOH, the pH of the resulting solution would be
Baking soda is
Which one of the following substances will be a mixed salt ?
Which is a basic salt
In hydrolysis of a salt of weak acid and strong base, A – + H 2 O ⇌ HA + OH – , the hydrolysis constant K h is equal to
Which of the following 0.1 M solution will contain the largest concentration of hydroniumions ?
1 M NaCl and 1 M HCl are present in an aqueous solution. The solution is
The compound whose 0.1 M solution is basic is
The solubility of A 2 X 5 is x mole dm – 3 . Its solubility product is
If K sp for HgSO 4 is 6 . 4 × 10 – 5 , then solubility of this substance in mole per m 3 is
When equal volumes of following solution are mixed, precipitation of AgCl ? K sp = 1 . 8 × 10 – 10 will occur only with
Let the solubilities of AgCl in pure water be 0.01 M CaCl 2 , 0.01 M NaCl and 0.05 M AgNO 3 be s 1 , s 2 , s 3 and s 4 respectively. What is the correct order of these quantities ? Neglect any complexation.
Which of the following statements is incorrect for a solution saturated with AgCl and AgBr if their solubilities in moles per litre in separate solutions are x and y respectively ?
Which of the following is most soluble in water ?
Solubility of BaF 2 in a solution of Ba NO 3 2 will be represented by the concentration term
At 30 0 C the solubility of Ag 2 CO 3 K SP = 8 × 10 – 12 would be greatest in one litre of
p H of the mixture containing 200ml of 0.1M CH 3 COOH and 100ml of 0.15M KOH is p k a of CH 3 COOH = 4 . 8
Solubility of AgCl is minimum in
The volume of the water needed to dissolve 1 g of BaSO 4 K SP = 1 . 1 × 10 – 10 at 25 0 C is
Silver nitrate solution is gradually added to an aqueous solution containing 0.01 M each of chloride, bromide and iodide ions. The correct sequence in which the halides will be precipitated is
Solubility product of AgCl is 2 . 8 × 10 – 10 at 25 0 C . Calculate solubility of the salt in 0.1 M AgNO 3 solution
The K SP of Mg OH 2 is 1 × 10 – 12 . 0.01 M Mg OH 2 will precipitate at the limiting pH
A solution of Na 2 CO 3 is added drop by drop to litre of a solution containing 10 – 4 mole of B a 2 + a n d 10 – 5 mole of Ag + , if K SP for BaCO 3 is 8 . 1 × 10 – 9 and K SP for Ag 2 CO 3 is 6 . 9 × 10 – 12 then which is not true
Solubility of calcium phosphate (molecular mass, M) in water is W g per 100 mL at 25 0 C . Its solubility product at 25 0 C will be approximately
M OH X has K SP 4 × 10 – 12 and solubility 10 – 4 M . The value of x is
The solubility product of chalk is 9 . 3 × 10 – 8 . Calculate its solubility in gram per litre
A salt M 2 X 3 dissolves in water such that its solubility is x g. mole/liter. Its K SP is
The precipitate of CaF 2 K sp = 1 . 7 × 10 – 10 is obtained when equal volumes of the following are mixed
If the solubility product of MOH is 1 × 10 – 10 mol 2 dm – 6 , then pH of its aqueous solution will be
K sp of a sparingly soluble salt AB 2 is 4 × 10 – 12 mol 3 L – 3 . The solubility of the salt is
In a saturated solution of the sparingly soluble strong electrolyte AgIO 3 (molecular mass = 283) the equilibrium which sets is AgIO 3 s ⇌ Ag + aq + IO 3 – aq If the solubility product constant K S P o f A g I O 3 at a given temperature is 1 . 0 × 10 – 8 , what is the mass of AgIO 3 contained in 100 mL of its saturated solution ?
The K SP for Cr OH 3 is 1 . 6 × 10 – 30 . The molar solubility of this compound in water is
At 25 0 C , the solubility product of Mg OH 2 is 1 . 0 × 10 – 11 . At which pH, will Mg 2 + ions start precipitating in the form of Mg OH 2 from a solution of 0.001 M Mg 2 + ions ?
Solid Ba NO 3 2 is gradually dissolved in a 1 . 0 × 10 – 4 M Na 2 CO 3 solution. At what concentration of Ba 2 + , will a precipitate begin to form ? K SP for BaCO 3 = 5 . 1 × 10 – 9
A buffer solution contains 1 mole of NH 4 2 SO 4 and 1 mole of NH 4 OH K b = 10 – 5 . The pH of solution will be
pH of a solution of 10 ml. 1 N sodium acetate and 50 ml 2 N acetic acid K a = 1 . 8 × 10 – 5 is approximately
Buffer capacity of a buffer solution is x, the volume of 1 M NaOH added to 100 mL of this solution if the change of pH by 1 is
What % of the carbon in the H 2 CO 3 – HCO 3 – buffer should be in the form of HCO 3 – so as to have a neutral solution ? K a = 4 × 10 – 7
The buffer solution of 100 ml having a pH value 4 when added to 1 ml dilute HCl, then the pH of buffer solution
Calculate the amount of NH 4 2 SO 4 in grams which must be added to 500 ml of 0.2 M NH 3 to yield a solution of pH = 9, K b for NH 3 = 2 × 10 – 5
What amount of sodium propanoate should be added to one litre of an aqueous solution containing 0.02 mole of propanoic acid K a = 1 . 0 × 10 – 5 at 25 0 C to obtain a buffer solution of pH 6
20 ml of 0.2 M NaOH is added to 50 ml, of 0.2 M CH 3 COOH to give 70 ml, of the solution. What is the pH of the solution ? The ionization constant of acetic acid is 2 × 10 – 5
Which one of following acts as Lewis acid but not as a Lewis base
Calculate pH of a solution of given mixture (0.1 mole CH 3 COOH + 0 . 2 mole CH 3 COONa ) in 100 ml of mixture. K = 2 × 10 – 5 .
What amount of HCl will be required to prepare one litre of a buffer solution of pH 10.4 using 0.01 mole of NaCN ? Given K ion HCN = 4 . 1 × 10 – 10 .
0.1 mole of CH 3 NH 2 K b = 5 × 10 – 4 is mixed with 0.08 mole of HCl and diluted to one litre. The H + in solution is
The pK a of a weak acid (HA) is 4.5. The pOH of an aqueous buffered solution of HA in which 50% of the acid is ionized is
A volume of 50.00 mL of a weak acid of unknown concentration is titrated with 0.10 M solution of NaOH. The equivalence point is reached after 39.30 mL of NaOH solution has been added. At the half-equivalence point (19.65 mL), the pH is 4.85. Thus, initial concentrations of the acid and its p K a values are
An indicator is a weak acid and pH range of its colour is 3 to 5. If the neutral point of the indicator lies in the centre of the H + corresponding to given pH range, then pH at the equivalence point is
Strong acids are generally used as standard solution in acid-base titrations because
At 25 o C pH range of phenolphthalein is 8 – 10. At 100 o C pH range of phenolphthalein would be
100 mL of 0.02 M benzoic acid pK a = 4 . 2 is titrated using 0.02 M NaOH. pH values after 50 mL and 100 mL of NaOH have been added are
When 10 ml of 0.1 M acetic acid p K a = 5 . 0 is titrated against 10 ml of 0.1 M ammonia solution p K b = 5 . 0 , the equivalence point occurs at pH
What will be the pH at the equivalence point during the titration of a 100 mL 0.2 M solution of CH 3 COONa with 0.2 M solution of HCl ? K a = 2 × 10 – 5 .
20 mL of a weak monobasic acid (HA) requires 20 mL 0.2 M NaOH for complete titration. If pH of solution upon addition of 10 mL of this alkali to 25 mL of the above solution of HA is 5.8. The pK a of the weak acid is
An acid-base indicator which is a weak acid has a p K I n value = 5.45. At what concentration ratio of sodium acetate to acetic acid would the indicator show a colour half-way between those of its acid and conjugate base forms ? [ P K a of acetic acid = 4 . 75 ]
An indicator has pK In = 5 . 3 . In a certain titration, this indicator is found to be 20% ionized in its acid form. Thus, pH of the solution is
A certain indicator (an organic dye) has pK a = 5 . For which of the following titrations may it be suitable.
An acid-base indicator which is a weak acid has a p H value = 5.5. At what concentration ratio of sodium acetate to acetic acid would the indicator show a colour, half-way between those of its acid and conjugate base forms ? pK a of acetic acid = 4.75
A weak acid (HA) after treatment with 12 mL of 0.1 M strong base (BOH) has a pH of 5. At the end point, the volume of same base required is 27 mL. K a of acid is (log 2 = 0.3)
What is the difference in pH for 1/3 and 2/3 stages of neutralization of 0.1 M CH 3 COOH with 0.1 M NaOH ?
Statement 1 : Ionic product is used for any types of electrolytes whereas solubility product is applicable only to sparingly soluble salts. Statement 2 : Ionic product is defined at any stage of the reaction whereas solubility product is only applicable to the saturation stage.
Statement 1 : The pH of a basic buffer mixture is given by : pH = pK a + log Base conjugate acid Statement 2 : The pH of an acidic buffer mixture is given by : pH = pK a + log conjugate base Acid
Statement 1 : The pH of pure water is less than 7 at 60 0 C . Statement 2 : As the temperature increases, pure water becomes slightly acidic.
Statement 1 : The pH of human blood at body temperature is found to be 6.9. Statement 2 : Blood is alkaline in nature.
Statement 1 : On passing HCl(g) through a saturated solution of Ba ( OH ) 2 a white turbidity appears. Statement 2 : The common ion effect is responsible for white turbidity.
Statement 1 : Degree of hydrolysis and pH of a salt, e.g., NH 4 CN is independent of concentration of NH 4 CN . Statement 2 : The solution of NH 4 CN in water has pH slightly greater than 7.
Statement 1 : In a pair of two electrolytes one having higher value of K sp is more soluble in water than the other having lower value of K sp . Statement 2 : Solubility of electrolyte depends upon K sp as well as on the nature of electrolyte.
Statement 1 : HgCl 2 and SnCl 2 cannot coexist in a solution. Statement 2 : Increase in concentration of Cl – in solution brings in precipitation of either of them.
Statement 1 : The solubility of HgI 2 in water deceases in presence of KI. Statement 2 : HgI 2 is insoluble in water but it becomes soluble in KI(aq).
Statement 1 : The dissociation constant of water at 60 0 C is 10 – 13 . Statemnet 2 : The pH of water is 6.5 and that it behaves as acid at 60 0 C
Statement 1 : In a titration of weak monoprotic acid with strong base, the pH at the half equivalent point is pK a . Statement 2 : At half equivalence point, it will form acidic buffer at its maximum capacity where [acid] = [salt].
Statement 1 : The H 3 O + has additional water molecules closely associated with it. Statement 2 : In solid state the species H 5 O 2 + and H 9 O 4 + have been found to exist.
Statement 1 : The proton transfer reaction between NH 3 and H 2 O proceeds only to a slight extent. Statement 2 : Proton transfer reaction is virtually complete in the case of HCl in dilute solution.
Statement 1 : Aqueous solutions of all strong acids contain only the same acid, the hydronium ion. Statement 2 : Hydronium ion is the strongest acid that can exist in any significant concentration in dilute aqueous solution.
Statement 1 : CHCl 3 is more acidic than CHF 3 . Statement 2 : The conjugate base of CHCl 3 is more stable than CHF 3
pH of Ba OH 2 solution is 12. Its solubility product is
The hydrolysis constant for ZnCl 2 will be
pH of a mixture of 1 M benzoic acid pK a = 4 . 20 and 1 M C 6 H 5 COONa is 4.5. In 300 ml buffer, benzoic acid is [log 2 = 0.3]
Equimolar solutions of the following were prepared in water separately. Which one of the solutions will record the highest pH ?
The dissociation constant of a weak acid is 1 . 0 × 10 – 5 , the equilibrium constant for the reaction with strong base is
The pH of 0.1 M solution of the following salts increases in the order
In the equilibrium A – + H 2 O ⇌ HA + OH – K a = 1 . 0 × 10 – 5 . The degree of hydrolysis of 0.001 M solution of the salt is
Which of the following is correct for a base?
For a weak acid HA with dissociation constant 10 – 9 , pOH of its 0.1 M solution is
The concentration of H + and concentration of OH – of a 0.1 aqueous solution of 2% ionized weak acid is [Ionic product of water = 1 × 10 – 14 ]
The values of K sp for CuS, Ag 2 S and HgS are 10 – 31 , 10 – 42 and 10 – 54 respectively. The correct order of their solubility in water is
If 50 ml of 0.2 M KOH is added to 40 ml of 0.5 M HCOOH, the pH of the resulting solution is K a = 1 . 8 × 10 – 4
What is the pH of a 1 M CH 3 COOH a solution K a of acetic acid = 1 . 8 × 10 – 5 ? K = 10 – 14 mol 2 litre – 2
A monoprotic acid in 0.1 M solution has K a = 1 . 0 × 10 – 5 . The degree of dissociation for acid is
By adding 20 ml 0.1 N HCl to 20 ml 0.001 N KOH, the pH of the obtained solution will be
The solubility product of a sparingly soluble salt AB at room temperature is 1 . 21 × 10 – 6 . Its molar solubility is
Which of the following pairs constitutes buffer ?
H 2 S gas when passed through a solution of cations containing HCl precipitates the cations of second group in qualitative analysis but not those belonging to the fourth group. It is because
At 25 0 C , the dissociation constant of a base BOH is 1 . 0 × 10 – 12 . The concentration of hydroxyl ions in 0.01 x M aqueous solution of the base would be
Which of the following can act as an acid and as a base ?
At certain temperature, p H of 0.01N Ba OH 2 is 11.699. Ionic product of water a that at temperature is
Select the incorrect statement out of the following.
The ionization constant of HF is 3 . 2 × 10 – 4 . Which of the following is the correct value of degree of dissociation if concentration is 0.02 M?
The P H of 0.1 M monobasic acid is 4.5. The K a and P K a values, respectively, are
Conjugate acid of peroxide ion is
At 298K, the magnitude of solubility product of two sparingly soluble salts ‘ AB ’ and ‘ AB 2 ‘ is same ( 4 × 10 – 12 ) . Based on this data the correct statement is
Statement 1 : If 200 mL of 0.1 N NaOH is added to 200 mL of 0.1 N H 2 SO 4 solution, then the resulting solution is acidic. Statement 2 : If milliequivalent of acid is greater than milliequivalnts of base, then upon mixing the solution is acidic.
Which of the following is not an example of an acid buffer?
What is the solubility of A 2 + 3 B 3 – 2 in water at 298 K?
What is the solubility of A x + y B y – x in water at 298 K?
Modern theories of acids and bases are very important in understanding acidic nature and basic nature. Which statement about these theories is false
Statement-I: The acid-base pair that differs only by one proton is called a conjugate acid-base pair. Statement-II: If Bronsted acid is a strong acid then its conjugate base is a weak base and vice-versa.
K α 1 , K a 2 and K a 3 are the respective ionisation constants for the following reactions. H 2 S ⇌ H + + HS – HS – ⇌ H + + S 2 – H 2 S ⇌ 2 H + + S 2 – The correct relationship between K α 1 , K a 2 and K a 3 is
Statement 1: The aqueous solution of FeCl 3 is basic in nature. Statement 2: FeCl 3 hydrolyses in water.
Statement 1: The solubility of salts of weak acid and strong base increases with increase in p H . Statement 2: At lower pH, equilibrium shifts in forward direction in the ionization of salt of weak acid and strong base
0.4 grams of sodium hydroxide is dissolved in 500 ml solution. The solution is now diluted by adding 500 ml of water. p H of the resultant solution is
Molar solubility of a salt, AB 2 is 3 × 10 – 6 M . Solubility product of the salt is
Which of the following is a Lewis acid?
P H of an acidic buffer is 5.8. p ka of weakacid is 4.8. 100 ml of 1M BA(salt) is mixed with ‘V’ ml of 0.1 M weakacid (HA). Value of ‘V’ is
K sp of a spraingly soluble salt, X 2 Y 3 in terms of molar solubility(s) is equal to
R-I : NH 3 + BF 3 H 3 N BF 3 R-II : NH 3 + H + NH 4 + Correct statements about R-I and R-II are A) NH 3 is a Lewis base in both R-I and R-II B) NH 3 is a B-L base in both R-I and R-II C) NH 3 is a Lewis base only in R-I D) NH 3 is a Lewis base only in R-II E) NH 3 is a B-L base only in R-II F) NH 3 is a B-L base only in R-I
p H of 0.1 M weak mono acidic base is 11. Dissociation constant of the base is
Which of the following is not a Lewis acid
Solubility product of AgCl is 1 . 8 × 10 – 10 M 2 . Molar solubility of AgCl in 0.1 M NaCl solution will be
Regarding the hydrolysis of one mole of Ferric chloride correct statement is
At 298 K, the p H of mixture containing 1000 ml of 0.1 M H 2 SO 4 and 500 ml of 1.2 M NH 4 OH is (p k b of NH 4 OH = 4.77)
When CH 3 COOC 2 H 5 was hydrolysed in presence of the rate constant obtained as 5 .40 × 10 − 5 s − 1 .But when 0 .1 MH 2 SO 4 was fused for hydrolysis, the rate constant obtained as 6 .20 × 10 − 5 s − 1 . From these it can be said that
Strong acid dissociates completely in water, the resulting base formed would be very weak. The reason is that
The extent of dissociation of an acid depends on
The process of interaction between water and cations/anions or both of salts is called
A mixture of acetic acid and sodium acetate acts as buffer solution around pH P and a mixture of ammonium chloride and ammonium hydroxide acts as a buffer around pH Q . P and Q respectively are
How many litres of water must be added to I L of an aqueous solution with a pH of 1 to create an aqueous solution of pH of 2?
Assuming complete ionisation, the pH of 0.1 M HCI is 1. The molarity of H 2 SO 4 with the same pH is
The pH of a mixture when a 50 mL solution of pH = I is mixed with a 50 mL of pH =2 is
The pK b for fluoride ion at 25°C is 10.83, the ionisation constant of hydrofluoric acid at this temperature is
The pK a of acetic acid and pK b of ammonium hydroxide are 4.76 and 4.75 respectively. Calculate the pH of ammonium acetate solution.
A weak base BOH is titrated with a strong acid HA. When 10 mL of HA is added, pH is found to be 9.00 and when 25 mL is added, pH is 8.00. The volume of the acid required to reach the equivalence point is
Point out the correct order of acidic strength in the same row of the periodic table.
In the following observation. Acid K a 1 K a 2 (X) Oxalic acid 5 . 9 × 10 – 2 6 . 4 × 10 – 5 Ascorbic acid 7 . 4 × 10 – 4 1 . 6 × 10 – 12 Sulphurous acid 1 . 7 × 10 – 2 6 . 4 × 10 – 8 (Y) Very large 1 . 2 × 10 – 2 Carbonic acid 4 . 3 × 10 – 7 (Z) Citric acid 7 . 4 × 10 – 4 1 . 7 × 10 – 5 4 . 0 × 10 – 7 Phosphoric acid 7 . 5 × 10 – 3 6 . 2 × 10 – 8 4 . 2 × 10 – 13 X,Y and Z respectively are
Point out the correct relation between K a , K b and K w
Which of the following relations is correct?
Which one of the following statements is incorrect?
A 0.01 M ammonia solution is 5% ionised. The concentration of OH – ion is
A 0.2 molar solution of formic acid is 3.2% ionised. Its ionisation constant is
If the ionisation constant of acetic acid is 1 . 8 × 10 – 5 at what concentration will it be dissociated to 2%?
The ionisation of weak base M OH can be represented by equation, MOH ( aq ) ⇌ M + ( aq ) + OH – ( aq ) K b = M + OH – / [ MOH ] where, K b is represented as
The concentration of hydrogen ion in a sample of soft drink is 3 . 8 × 10 – 3 M . What is its pH?
At 363K, pure water has H 3 O + = 10 – 6 M . The value of K w at this temperature will be
Hydronium ion concentration in molarity is more conveniently expressed on a logarithmic scale known as the
In the following reaction, H 2 O ( l ) Acid + H 2 O ( l ) X ⇌ H 3 O + conjugate acid ( aq ) + OH – Y ( aq ) X and Y respectively are
Which of the following are the conjugate bases of the given acids? HClO 4 , HCl , HBr , HI , HNO 3 and H 2 SO 4
The correct order of increasing H 3 O + in the aqueous solution is
What is the decreasing order of strength of the bases OH – , NH 2 – , H – C ≡ C – and CH 3 – CH 2 – ?
A buffer solution is a solution whose pH value on keeping in the air
I mL of N/100 HCI is added to 1 L of buffer having pH = 5. The pH of the solution will be
Which of the following is correct regarding buffer sol?
100 mL of a solution contains 0.1 M 0 . 1 MNH 4 OH and 0 . 1 MNH 4 Cl . The pH of the solution will not change on adding.
A buffer solution is prepared in which the conc. NH 3 is 0.30 M and the concentration of NH 4 + is 0.20 M. If the equilibrium constant, K b for NH 3 equals 1 . 8 × 10 – 5 , what is the pH of this solution
The pK a of HCN is 9.30. The pH of a solution prepared by mixing 2.5 moles of KCN and 2.5 moles of HCN in water and making up the total volume of 500 mL is
A 100 mL, 0.1 M solution of ammoniurn acetate is diluted by adding 100 mL of water. The pH of the resulting solution will be ( pK a of acetic acid is nearly equal to pK b of NH 4 OH )
One litre of a buffer solution containing 0.01 M NH 4 Cl and 0.1 M NH 4 OH having pK b of 5 has pH of
Calculate pH of 0.10 N acetic acid having K a = 1 . 8 × 10 – 5
2g of NaOH is dissolved in water to make 1L solution. What is the pH of solution?
The pH 0.005 M codeine ( C 18 H 21 NO 3 ) solution is 995. Its pK b value is
What will be the range of solubility of slightly soluble salts?
What will be the molar solubility S of a solid salt with general formula M x p + X y q – ?
What will be the conjugate bases for the following Bronsted acids? HF , H 2 SO 4 and HCO 3 –
Point out the conjugate acids for the following Bronsted bases NH 2 – , NH 3 and HCOO – .
Choose the correct one which is the weakest acid.
Carboxylic acids readily dissolve in aqueous sodium bicarbonate, liberating carbon dioxide. Which one of the following is correct?
Which equilibrium can be described as an acid-base reaction using the Lewis acid-base definition, but not using Bronsted-Lowry definition?
The addition of NaCl to AgCl decreases the solubility of AgCl because
The solubility product of a sparingly soluble salt AB at room temperature is 1 . 21 × 10 – 6 , its molar solubility is
The solubility product K sp of AgCl is 1 . 8 × 10 – 10 . Precipitation of AgCl will occur only when equal volumes of solutions of
The solubility product K sp of the sparingly soluble salt Ag 2 CrO 4 is 4 × 10 – 12 . The molar solubility of the salt is
Solubility of calcium phosphate (molecular mas s, M) in water is W g per 100 mL at 25°C, Its solubility product at 25°C will be approximately.
The addition of NaCl to AgCl decreases the solubility of AgCl because
Calculate the molar solubility of Ni ( OH ) 2 in 0.10 M NaOH. The ionic product of Ni ( OH ) 2 is 2 . 0 × 10 – 15 .
pH of saturated solution of Ba ( OH ) 2 is 12.The value of solubility product of K sp of Ba ( OH ) 2 is
Calculate the solubility of A 2 X 3 in pure water, assuming that neither kind of ion reacts with water. The solubility product of A 2 X 3 , K sp = 1 . 1 × 10 – 23
At 20°C, the Ag + ion concentration in a saturated solution of Ag 2 CrO 4 is 1 . 5 × 10 – 4 mol / L . At 20°C, the solubility product of Ag 2 CrO 4 will be
Calculate the solubility of silver phosphate (Ag 3 PO 4 ) in 0.1M AgNO 3 (k SP Ag 3 PO 4 = 1.1 X 10 -16 )
Statement I: Michael Faraday classified the substances into two categories based on their ability to conduct electricity. Statement II: One category of substances conduct electricity in their aqueous solutions and are called electrolytes, while the other do not and are thus, referred to as non-electrolytes.
Statement I: The equilibrium moves in the direction of the formation of weaker acid and weaker base. Statement II: The reason is that stronger acid donates a proton to the stronger base.
Statement I: Higher order ionisation constant ( K a 2 , K a 3 are smaller than the lower order ionisation constant ( K a 1 ) of a polyprotic acid. Statement II: It is more difficult to remove a positively charged proton from a negative ion due to electrostatic forces.
Statement I: Common ion effect is defined as a shift in equilibrium on adding a substance that provides more of an ionic species already present in the dissociation equilibrium. Statement II: Common ion effect is a phenomenon which can be explained on the basis of Le-Chatelier’s principle.
Statement I: An aqueous solution of ammonium acetate can act as a buffer. Statement II: Acetic acid is a weak acid and NH 4 OH is a strong base
Statement I: BF 3 is weaker Lewis acid than BCl 3 . Statement II: The planar BF 3 molecule is stabilised to a greater extent than BCl 3 by B – X back bonding.
Statement(I): Aqueous solution of ammonium carbonate is acidic. Statement(II): Acidic/basic nature of solution of a salt of weak acid and weak base does not depends on K a and K b value of the acid and the base forming it.
Which is the set of amphoteric species compounds?
Solubility of M OH 2 in 0.1 M NaOH is K sp of M OH 2 = 2 × 10 – 24 M 3
Four grams of NaOH is dissolved in hundred litre solution. At 298 K, p H of the solution is
0.1 moles of HCl is dissolved in hundred litre solution. At 298 K, p H of the solution is
The weakest base among the following species is
Equal volumes of 0.15M Sulphuric acid and 0.2M Potassium hydroxide are mixed. p H of resultant mixture is
Solubility product of Silver chloride is 10 – x M 2 . Solubility of Silver chloride is 1 . 435 × 10 – 3 g / litre . Value of ‘ x ‘ is
p H of mixture containing two moles of NH 4 OH and half mole of H 2 SO 4 is p K b of NH 4 OH = 4 . 8
Molar solubility of M OH 2 in 0.2 M NaOH will be K sp of M OH 2 = 2 × 10 – 24 M 3
To a one litre solution containing 8 grams of sodium hydroxide, 14.7 grams of sulphuric acid is added. p H of the solution at 298 K is
Solubility product of Silver chloride is 10 – 10 M 2 . Solubility of Silver chloride is 1435 × 10 – x g / litre . Value of ‘ x ‘ is
The weakest base among the following is
Equal volumes of 0.2 M Sulphuric acid and 0.2 M Potassium hydroxide are mixed. p H of resultant mixture is
Regarding aqueous solution of Potassium Cyanide, correct statements are A) Solution is alkaline in nature B) It undergoes anionic hydrolysis C) It remains colourless by the addition of Phenolpthalein D) Its hydrolysis constant depends on K a of weak acid
Solubility of AgCl is minimum in
The conjugate base of H 2 PO 4 – is ;
Which is the set of amphiprotic species?
For pure water :
The pH of a solution is 5. To this solution acid was added so that its pH value be comes 2.0. The increase in H’ concentration is :
P OH of 0.002 M HNO 3 . is :
4.0 g of Na OH and 4.9 g of H 2 SO 4 are dissolved in water and volume is made upto 250 mL. the pH of this solution is :
What is the pH of a solution in which 25.0 mL of O.I M NaOH is added to 25 mL of O.08M HCI and final solution is diluted to 500 mL?
H + ion concentration of water does not change by adding :
K sp of Zr 3 PO 4 4 in terms of solubility (S) is
K sp of AgCl is 1 × 10 – 10 . Its solubility in 0.1 M KNO 3 will be:
